Chem 1030 Test 2 Study Guide
1- Name the ionic compounds:
2- Name the covalent compounds:
d. N2O3 Don't forget about the age old question of How will you define prokaryotic cells?
g. NH3 If you want to learn more check out What are the advantages and disadvantages of market systems?
3- Write the chemical formulas for the following compounds: a. Sodium Chloride
b. Ammonium Carbonate We also discuss several other topics like Operational definition refers to what?
c. Potassium Hydroxide
d. Calcium (II) Sulfate
e. Zinc (II) Phosphate
f. Iron (III) Nitrate
g. Cobalt (III) Phosphate
h. Iron (II) Sulfate
i. Magnesium (II) Hydroxide
j. Potassium Chloride
4- Name three polyatomic ions.
5- Know the following prefixes:
a. Mono f. Hexa
b. Di g. Hepta
c. Tri h. Octa
We also discuss several other topics like What is clitoral prepuce?
d. Tetra i. Nona
e. Penta j. Deca
6- Define and give three examples of a compound.
7- What information does a Lewis Dot Symbol provide?
8- Give the Lewis Dot Symbols for Be, Ca, Li+ and Sr2+.
9- What is ionic bonding?
10-What is the relationship between ionization energy, electron affinity, and the formation of ionic compounds?
11-What is Lattice Energy and what does it indicate about stability?
12-An ionic bond is formed between cation A+ and anion B-. Based on Coulomb’s Law how would the energy of the ionic bond be affected by the following changes:
a. Doubling the radius of A+
b. Tripling the charge on A+
c. Doubling the charges on A+ and B
d. Decreasing the radii of A+ and B- by half
13-Use Lewis Dot Symbols to show the transfer of electrons between Na and F, and Ba and O to form cations.
14-What are the laws of definite proportions and multiple proportions? 15-What are the two most commonly used molecular models? 16-Define molecular and empirical formula, and describe the similarities and differences between them. Don't forget about the age old question of What is the difference between plant and animals?
17-Give the empirical formula for the following compounds.
a. P4O10 d. C5H12O
b. C10H22 e. N2O4
18-Give the molecular formula for the following compounds.
a. CH2 d. NO2
b. Na2CO3 e. Fe2O3
20-What’s the difference between an inorganic compound and an organic compound?
21-What is the difference between molecular mass and formula mass? What type of compound does each refer to?
22-Calculate the molecular mass in the following compounds. a. C6H6O d. CH3Cl
b. H2SO4 e. SO2
23-Calculate the formula mass in the following compounds.
a. NF2 d. K2SO4
b. Al2O3 e. SO3
c. Fe(NO3)3 Don't forget about the age old question of What is the meaning of bond energy?
24-Define percent composition.
25-Calculate the percent composition by mass of each of the elements in the following compounds.
26-True or False. Molar Mass is numerically equivalent to Molecular Mass for a covalent compound, although the units are different.
27-Calculate the Molar Mass of the following compounds.
28-How many molecules are of C2H6 are present in 0.334 g of C2H6? 29-Calculate the number of C, H and O atoms in 1.5 g of glucose. 30-How many moles of Fe are present in 1 kg of the compound Fe2O3? 31-Explain the octet rule.
32-Define and show how to represent the following bonds. a. Single
33-How does the bond length change between bonds? How does bind length relate to bond strength?
34-For each of the following pairs, state whether they will form an ionic or covalent bond.
a. I and Cl
b. Mg and F
c. B and F
d. K and Br
35-Define electronegativity and electron affinity. Explain their trend on the periodic table.
36-What is a polar covalent bond? Give two examples.
37-List the following bonds in order of increasing ionic character: carbon to hydrogen, fluorine to hydrogen, bromine to hydrogen, sodium to chlorine, potassium to fluorine, lithium to chlorine.
38-Label the following bonds as ionic, polar covalent, or nonpolar covalent. a. The CC bond in H3CCH3
b. The KI bond in KI
c. The NB bond in H3NBCl3
39-Draw Lewis Structures for the following compounds.
40-What is a formal charge?
41-Draw Lewis Structures for the following ions and show formal charges. a. NO2+
42-What are resonance structures?
43-Draw two resonance structures for the following.
44-Give three examples of compounds that do not satisfy the octet rule, and draw a Lewis Structure for each.
45-Draw Lewis Structures for SbCl5 and BrO2.